64ml of nitric acid required fr one litre
The amount of NaOH used in a titration depends on the volume and concentration of the NaOH solution used in the experiment. To calculate the exact amount of NaOH used, you would need to know the molarity of the NaOH solution and the volume used in the titration.
Molarity = moles of solute/volume of solution 0.53 M NaOH = moles NaOH/3.8 Liters = 2.014 moles, or about 80 grams
A 50% purity solution of NaOH would contain 500 grams of NaOH per liter of solution. Given that the density is 1.53 g/mL, there would be approximately 327.5 grams of NaOH in one liter of solution (1.53 g/mL * 1000 mL).
First you must either know how much 50% NaOH you want to start with or know how much 2% NaOH you need at the end. Let's say you want 1L of the 2% NaOH. Use this equation, and solve for x, where in this case, x is the volume of 50% NaOH needed. (50% NaOH)x = (2%) * 1000 ml 0.5x = 0.02(1000) x = 20/0.5 = 40 Therefore, 40 ml of 50% NaOH in 960 ml water will produce 2% NaOH. Use a 1000 ml volumetric flask to be most precise.
To calculate the amount of NaOH in the solution, multiply the volume (4.7 L) by the molarity (0.57 mol/L). Amount of NaOH = Volume (L) x Molarity (mol/L) = 4.7 L x 0.57 mol/L = 2.679 moles of NaOH.
The amount of NaOH used in a titration depends on the volume and concentration of the NaOH solution used in the experiment. To calculate the exact amount of NaOH used, you would need to know the molarity of the NaOH solution and the volume used in the titration.
Molarity = moles of solute/volume of solution 0.53 M NaOH = moles NaOH/3.8 Liters = 2.014 moles, or about 80 grams
A 50% purity solution of NaOH would contain 500 grams of NaOH per liter of solution. Given that the density is 1.53 g/mL, there would be approximately 327.5 grams of NaOH in one liter of solution (1.53 g/mL * 1000 mL).
First you must either know how much 50% NaOH you want to start with or know how much 2% NaOH you need at the end. Let's say you want 1L of the 2% NaOH. Use this equation, and solve for x, where in this case, x is the volume of 50% NaOH needed. (50% NaOH)x = (2%) * 1000 ml 0.5x = 0.02(1000) x = 20/0.5 = 40 Therefore, 40 ml of 50% NaOH in 960 ml water will produce 2% NaOH. Use a 1000 ml volumetric flask to be most precise.
To calculate the amount of NaOH in the solution, multiply the volume (4.7 L) by the molarity (0.57 mol/L). Amount of NaOH = Volume (L) x Molarity (mol/L) = 4.7 L x 0.57 mol/L = 2.679 moles of NaOH.
I assume you mean molar instead of mole?Fast:The HCl solution is 3 times as concentrated.Since both can only donate 1 H+ or OH-...you wil need 3 times as much NaOH to neutralise the HCl.20 ml * 3 = 60 mlSlow:The HCl solution has 6 mol/LThere is 20 ml of it, so you have 0.02 L * 6 mol/L = 0.12 mol of HClEach mole of HCl donates 1 mole of H+So there is 0.12 mol of H+ that you have to neutralise.This equals to 0.12 mol OH-Each NaOH donates 1 OH-So you need 0.12 mol NaOHThe NaOH solution you are using has 2 mol/LSo you have to use 0.12 mol / 2 mol/L = 0.06 L = 60 ml
The amount of NaOH needed to raise the pH from 8 to 10 depends heavily on the conditions. The amount of NaOH needed will increase as the volume of the solution increases. Even more importantly, buffers can stabilize the pH significantly. If buffers are presently, the pH change will be much more gradual, and more NaOH will be required.
Well, honey, preparing a 5 N NaOH solution is as easy as pie. Just measure out the appropriate amount of NaOH pellets and dissolve them in water until you reach the desired volume. Make sure to wear your safety goggles and gloves, because nobody wants a chemical burn. And voilà, you've got yourself a 5 N NaOH solution ready to go.
The answer is 50 mL.
You need 40.01 g NaOH per liter volume of the solution. This is not the same as adding 1 liter of water to 40.01 g of NaOH. The NaOH must be put in the flask and the volume brought up to 1 liter total volume (NaOH volume + water volume).
There is 0.5 moles of NaOH per litre To calculate 0.5 molar NaOH first know the molecular weight of NaOH i.e 40 now multiply the number of moles of NaOH you have (0.5) found as above. so to find the number of grams of NaOH we needed to start with (0.5) * (40) = 20g So dissolve 20g of NaOH in one litre of the solution to prepare 0.5 molar solution
If you have a standard solution of an acid, like hydrochloric or sulfuric, you can perform a titration in the presence of phenolphtalein or methyl orange and calculate the solution's normality or, you can weigh a sample of a strong solid acid ( orthoiperiodic acid or even oxalic acid), titrate the acid with the hydroxide solution, again in the presence of phenolphtalein or methyl orange and calculate the concentration of NaOH. If you want to have a solution with an exact concentration, let's say 1 molar, and the actual concentration is 1,33 molar, you simply calculate how much water you need to ad in a specific quantity of solution, to dilute it to exactly 1 molar.